Exam on Gas Thermodynamics: Definitions, Equation of State, and Processes - Prof. Howard J, Exams of Physical Chemistry

Download Exam on Gas Thermodynamics: Definitions, Equation of State, and Processes - Prof. Howard J and more Exams Physical Chemistry in PDF only on Docsity! V EM Prof. DeVoe february 28, 1983 EXAM i NAME SIGNA3URE (reguired R = 8.314 J K"1 mol""1 1 atm « 1.013 x 105 Pa t/°C + 273.15 0.08206 dm3 atm K""1 mol""1 1 dm3 « 1 L - 10 3 m3 EACH QUESTION IS WDREH 20 POINIS 1. For each of the following, write a mathematical definition using symbols from the textbook: (a) partial pressure of component i in a gas mixture: p. ~ (b) compression factor: 2 = (c) reduced temperature: T = (d) isobaric coefficient of. thermal expansion: a = (e) total differential of internal energy with T and V taken as independent variables: dU = 2. A certain gas obeys the equation of state: pV = nRT(l + nB/V) where B is a constant at constant temperature. Derive an expression for the work done in an isothermal, reversible expansion of the gas from volume Vj to volume V-. Show all steps. GO CN TO PAGE 2 - >" - . , , '-2- ** f ' < In pjjoblems 3 - 5, the system contains 0.500 mol Xe with a constant-volume molar heat capacity value Cy = 12.48 J K nol . Assume perfect gas behavior. Show all work and write the final answers in the spaces provided. 3. The system described above is heated from 25.0 °C to 35.0 °C at a constant pressure of 1.00 atm. Calculate AU, AH, q, and w. ' AU = _________ AH - _________ q - ______ w = 4. The same system is initially at 1.000 atm and 25.0 C. It is expanded isothermally against an external pressure of 0.500 atm until its pressure equals the external pressure. Calculate AU, AH, q, and w. AU = AH * w 5. TSne same system is initially at 25.0 °C with a volume of 12.2 dm . It is compressed (reduced in volume) adiabatically using a constant external pressure of 2.00 atm until its temperature has increased to 125.0 °C. Calculate the final volume (Vf). Vf END OP EXAM